Transcript General Chemistry Principles & Modern Applications 9 th Edition

General Chemistry
Principles & Modern Applications
9th Edition
Petrucci/Harwood/Herring/Madura
Chapter 13
Solutions and their Physical Properties
Dr. Travis D. Fridgen
Memorial University of Newfoundland
© 2007 Pearson Education
Which one of the following would you expect to be most soluble in water?
2.
1.
4.
3.
5.
Which one of the following would you expect to be most soluble in water?
2.
1.
4.
3.
5.
Of the solvent/solute
pairs given to the right,
which of the solutes
would you expect to be
least soluble in the
solvent.
1.
in
2.
in
3.
in
Of the solvent/solute
pairs given to the right,
which of the solutes
would you expect to be
least soluble in the
solvent.
1.
in
2.
in
3.
in
In the process of refining crude oil, the fraction at the
top of the column is the one with the highest molecular
weight.
1. True
2. False
In the process of refining crude oil, the fraction at the
top of the column is the one with the highest molecular
weight.
1. True
2. False
If a diver surfaces too quickly from a dive,
N2(g) dissolved in the divers blood will be
released quickly resulting in a painful and
dangerous condition called the bends. This
is the same phenomenon as taking the top
of of a pop bottle as depicted to the right.
1. True
2. False
If a diver surfaces too quickly from a dive,
N2(g) dissolved in the divers blood will be
released quickly resulting in a painful and
dangerous condition called the bends. This
is the same phenomenon as taking the top
of of a pop bottle as depicted to the right.
1. True
2. False
The number of moles of CO2(g) above an aqueous solution of CO2 decreased
by two. The volume of gas above the solution is concurrently decreased by a
factor of two. The concentration of CO2 in solution
1. Decreases by a factor of 4.
2. Decreases by a factor of 2.
3. Remains the same.
4. Increases by a factor of 2.
5. Increases by a factor of 4.
The number of moles of CO2(g) above an aqueous solution of CO2 decreased
by two. The volume of gas above the solution is concurrently decreased by a
factor of two. The concentration of CO2 in solution
1. Decreases by a factor of 4.
2. Decreases by a factor of 2.
3. Remains the same.
4. Increases by a factor of 2.
5. Increases by a factor of 4.
To the right is a diagram of a closed system
containing two salt water solutions. The solution
labeled A is more concentrated than the one
labeled B. Which of the diagrams below best
represents the system at an infinite time after
preparation?
A
B
1.
A
B
2.
A
B
A
B
3.
To the right is a diagram of a closed system
containing two salt water solutions. The solution
labeled A is more concentrated than the one
labeled B. Which of the diagrams below best
represents the system at an infinite time after
preparation?
A
B
1.
A
B
2.
A
B
A
B
3.
Which of the following aqueous solutions will have
the highest boiling point?
1. 3 molal glucose
2. 4 molal ethanol
3. 2.5 molal NaCl
4. 2.5 molal CaCl2
5. Cannot tell without Kb for water
Which of the following aqueous solutions will have
the highest boiling point?
1. 3 molal glucose
2. 4 molal ethanol
3. 2.5 molal NaCl
4. 2.5 molal CaCl2
5. Cannot tell without Kb for water
A 2.0 molal aqueous solution of glucose
(C6O6H12) is found to boil at 101 oC. What
would the boiling point of a 2.0 molal
solution of sucrose be?
glucose (C6O6H12)
1. 102 oC
2. 100.5 oC
3. 101 oC
4. Slightly higher than 100.5 oC
5. Cannot determine without Kb
sucrose (C12O11H22)
A 2.0 molal aqueous solution of glucose
(C6O6H12) is found to boil at 101 oC. What
would the boiling point of a 2.0 molal
solution of sucrose be?
glucose (C6O6H12)
1. 102 oC
2. 100.5 oC
3. 101 oC
4. Slightly higher than 100.5 oC
5. Cannot determine without Kb
sucrose (C12O11H22)
The freezing point of a solution is
lower than that of the pure solvent
because
1. The addition of solute to the
liquid increases the rate of escape
of molecules from the solid phase to the liquid phase. At lower temperature
these rates can again become equal.
2. The addition of solute to the liquid decreases the rate at which solvent
molecules enter the solid phase. By lowering the temperature the rate of
escape of molecules from the solid to liquid phase is also lowered and
become equal.
The freezing point of a solution is
lower than that of the pure solvent
because
1. The addition of solute to the
liquid increases the rate of escape
of molecules from the solid phase to the liquid phase. At lower temperature
these rates can again become equal.
2. The addition of solute to the liquid decreases the rate at which solvent
molecules enter the solid phase. By lowering the temperature the rate of
escape of molecules from the solid to liquid phase is also lowered and
become equal.
As the water evaporates from this saturated
solution
1. the vapor pressure above the solution
increases.
2. the vapor pressure above the solution
decreases.
3. the vapor pressure above the solution
remains constant.
As the water evaporates from this saturated
solution
1. the vapor pressure above the solution
increases.
2. the vapor pressure above the solution
decreases.
3. the vapor pressure above the solution
remains constant.
Two aqueous solutions of equal volume, one containing 20 g of lactic acid
(C3H6O3) and one containing 10 g of glucose (C6H12O6) are separated by a
semi permeable membrane (allowing only H2O to pass). The net flow of
water through the membrane is?
1. Left
2. Right
3. There is no net flow.
4. Cannot tell without knowing the
exact volume of the solutions.
20 g C3H6O3
10 g C6H12O6
Two aqueous solutions of equal volume, one containing 20 g of lactic acid
(C3H6O3) and one containing 10 g of glucose (C6H12O6) are separated by a
semi permeable membrane (allowing only H2O to pass). The net flow of
water through the membrane is?
1. Left
2. Right
3. There is no net flow.
4. Cannot tell without knowing the
exact volume of the solutions.
20 g C3H6O3
10 g C6H12O6
The table to the right shows the experimental
van’t Hoff factor, i, for three electrolytes at 1.0
m and the expected value at infinite dilution.
Which of the following is the best explanation
for the increase in the difference in i at for the
salts shown?
1. The higher the charge on the ion, the
smaller the radius so only a fraction of the oppositely charged ions are
separated in solution. The rest are bound to one another.
2. The higher the charge on the ions, the greater attraction for ions of opposite
charge. The greater the attraction the less they dissolve.
3. The higher the charge on the ion, the greater attraction for oppositely
charged ions. The greater the attraction the more they act like a single
particle rather than separate particles.
The table to the right shows the experimental
van’t Hoff factor, i, for three electrolytes at 1.0
m and the expected value at infinite dilution.
Which of the following is the best explanation
for the increase in the difference in i at for the
salts shown?
1. The higher the charge on the ion, the
smaller the radius so only a fraction of the oppositely charged ions are
separated in solution. The rest are bound to one another.
2. The higher the charge on the ions, the greater attraction for ions of opposite
charge. The greater the attraction the less they dissolve.
3. The higher the charge on the ion, the greater attraction for oppositely
charged ions. The greater the attraction the more they act like a single
particle rather than separate particles.
The table to the right shows the
experimental van’t Hoff factor, i,
for three electrolytes at various
dilutions. Which of the following
is the best explanation for the
increase in i at greater dilution.
1. These ionic compounds don’t fully dissolve unless under very dilute conditions.
2. At greater dilution, there are less interactions between oppositely charged ions
so they act like completely separate entities.
3. At greater dilution, there are less forces holding the oppositely charged
particles together so they act like completely separate entities.
The table to the right shows the
experimental van’t Hoff factor, i,
for three electrolytes at various
dilutions. Which of the following
is the best explanation for the
increase in i at greater dilution.
1. These ionic compounds don’t fully dissolve unless under very dilute conditions.
2. At greater dilution, there are less interactions between oppositely charged ions
so they act like completely separate entities.
3. At greater dilution, there are less forces holding the oppositely charged
particles together so they act like completely separate entities.
The freezing point depression and boiling point depression constants for a
number of liquids are given in the table below. Without using a calculator, which
of the following solutions’ freezing point is decreased by the greatest amount
when 1 mole of solute is dissolved in 1 kg of the solvent?
1.
2.
3.
4.
5.
The freezing point depression and boiling point depression constants for a
number of liquids are given in the table below. Without using a calculator, which
of the following solutions’ freezing point is decreased by the greatest amount
when 1 mole of solute is dissolved in 1 kg of the solvent?
1.
2.
3.
4.
5.